For the chemical reaction shown below assume all products and reactants are in the aqueous phase. 2NO2 + 7H2 2NH3 + 4H20 If a chemist mixed 0.893 moles of NO2 with 1.837 moles of H2 in a 2.79 liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then he/she draws an air sample from an air port using a gas tight GC syringe and analyzes the sample and found 0.383 moles of NH3 then how many moles of H2O is present at equilibrium to 3 decimal places? Don't write the word moles after your 3 decimal place answer.
For the chemical reaction shown below assume all products and reactants are in the aqueous phase. 2NO2 + 7H2 2NH3 + 4H20 If a chemist mixed 0.893 moles of NO2 with 1.837 moles of H2 in a 2.79 liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then he/she draws an air sample from an air port using a gas tight GC syringe and analyzes the sample and found 0.383 moles of NH3 then how many moles of H2O is present at equilibrium to 3 decimal places? Don't write the word moles after your 3 decimal place answer.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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